Acids and Bases Flashcards
what is Arrhenius’s definition of a strong acid
A substance that almost completely dissociates in water to form H+ Ions
what is Arrhenius’s definition of a strong base
A substance that almost completely dissociates in water to form OH- Ions
what is Arrhenius’s definition of a acid
A substance that dissociate sin water to produce H+ ions
what is Arrhenius’s definition of a base
A substance that dissociate sin water to produce OH- ions
what is Arrhenius’s definition of a weak acid
A substance that partially dissociates to produce H+ ions
What is the Bronsted lowry definition of a base/
A proton acceptor
What is the Bronsted lowry definition of an acid
A proton donor
What is the Bronsted lowry definition of a strong base
A strong base is a good proton acceptor.
What is the Bronsted lowry definition of an a strong acid
A strong acid is a good proton donor
What is the Bronsted lowry definition of a weak acid
A weak acid is a poor proton donor.
What is the Bronsted lowry definition of a weak base
A weak base is a poor proton acceptor
how does an acid chnage into a conjugate base?
An acid changes into its conjugate base when it donates a proton.
how does a base change into a conjugate acid?
A base changes into its conjugate acid when it accepts a proton.
what is a conjugate acid-base pair?
A conjugate acid–base pair (conjugate pair) is any pair consisting of an acid and a base that differ by one proton
what is a salt?
A salt is the substance formed when the hydrogen ion from an acid is replaced by a metal or an ammonium ion
what is neutralisation?
Neutralisation is the reaction between an acid and abase to form a salt and water
Give an example of neutralization in daily lives?
Medicine. Hydrochloric acid is produced by the stomach to help digest food. Sometimes the stomach produces too much HCl and indigestion tablets are needed to neutralise the ph
Agriculture- If soils are too acid then lime is spread over the soil to increase the ph
Environment- In areas of acid rain the water is too acid for fish so adding limestone to lakes increase the ph so fish can survive
GIve three differences between Arrhenius and Bronsted lowry theory of acids and bases?
Arrhenius- Acids and bases are restricted to aqueous solutions.
Bases produce OH- when they dissociate in water.
Does not explain substances that are amphoteric
Bronsted Lowry- Acids and bases are not restricted to aqueous solutions they can involve reactions in the gaseous state
Not all bases produce OH- ions
It uses proton transfer to explain how some substances are amphoteric
Give some limitations o Arrhenius thery
Definitions are restricted to aqueous solutions
Water is amphoteric but according to him it cannot be amphoteric
H+ ions do not exist on their own in aqueous solutions
what does amphoteric mean
They can act as acids and bases depending on the reaction eg H20
Why is NH3 not considered a base according to Arrhenius but is by Bronsted LowrY?
BL- Says that it is a base as it is a proton acceptor
AH- Says that it is not a base as it does not dissociate in water to produce OH-
If an acid loses a proton it forms what
A conjugate base
If a base gains a proton is forms what
A conjugate acid
How would you know what is the acid to conjugate base pair
Hydrogens decrease by 1
Charge decreases by 1
